Weak electrolytes = few ions to carry the charges from one electrode to the other. Examples of weak electrolytes: Weak acids or bases (Ethanoic acid, aqueous ammonia)

Non-electrolytes = no ions available to carry the charges from one electrode to the other. Examples of non-electrolytes: Pure water, organic liquids or solvents

Electrodes are conductors through which electrons enter and leave the electrolyte.

Anode is the POSITIVE (+) electrode from which electrons leave the electrolyte (or the electric current enters the electrolyte)

Cathode is the NEGATIVE (-) electrode from which electrons enter the electrolyte (or the electric current leaves the electrolyte)

Electrodes are typically made up of inert materials (which do not participate in any redox reactions), such as carbon, platinum, titanium, or stainless steel. (NOTE: There are some cases where the electrodes undergoes redox reactions during electrolysis.)

What happens during electrolysis?

Negative ions (Anions) are attracted to the anode while the positive ions (cations) are attracted to the cathode.

When the ions reaches their respective electrodes, they will be discharged. (They lose or gain electrons and form neutral atoms)

Hence, at anode, anions are discharged through loss of electrons; while at the cathode, cations are discharged through gain of electrons.